Name _________________________________________ Hour______
Redox Review

Oxidation state rules:
o Anything by itself
o
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Heavenly 7
Important mnemonics:
o OIL RIG
o
Oxygen
o
Group 1
o
Hydrogen
o
Group 2
o
RED CAT
o
AN OX
Writing a balanced half reaction:
o In oxidation, electrons are written as ______________________
o
In reduction, electrons are written as ______________________
o
In a balanced reaction, the number of ______________________ must be equal!
Oxidation states:
Write the oxidation state of each of the following elements
Ca(SO4)2
Ca: ____
S: ____
NaI
Na: ____
I:____
Fe
Fe: ____
Mg(NO3)2
Mg: ____
O2
O: ____
N: ____
O: ____
O:____
Write whether each of the following is an example of oxidation or reduction and write a half reaction for each
Cu becomes Cu2+______________________ Half reaction: ____________________________
Sn4+ becomes Sn2+______________________ Half reaction: ____________________________
Cr3+ becomes Cr6+______________________ Half reaction: ____________________________
Ag becomes Ag+______________________ Half reaction: ____________________________
Cu + 2Ag(NO3) 2Ag + Cu(NO3)2
What is oxidized? ____
What is the oxidizing agent? ____
What is reduced? ____
What is the reducing agent?____
Write the oxidation half reaction: _____________________________
Write the reduction half reaction: _____________________________
Write the balanced half reaction: ______________________________
Draw what his happening:
2H2 + O2  2H2O
What is oxidized? ____
What is the oxidizing agent? ____
What is reduced? ____
What is the reducing agent?____
Write the oxidation half reaction: _____________________________
Write the reduction half reaction: _____________________________
Write the balanced half reaction: ______________________________
2FeO + C  2Fe + CO2
What is oxidized? ____
What is the oxidizing agent? ____
What is reduced? ____
What is the reducing agent?____
Write the oxidation half reaction: _____________________________
Write the reduction half reaction: _____________________________
Write the balanced half reaction: ______________________________
S + O2  SO2
What is oxidized? ____
What is the oxidizing agent? ____
What is reduced? ____
What is the reducing agent?____
Write the oxidation half reaction: _____________________________
Write the reduction half reaction: _____________________________
Write the balanced half reaction: ______________________________
NaNO3 + Pb  NaNO2 + PbO
What is oxidized? ____
What is the oxidizing agent? ____
What is reduced? ____
What is the reducing agent?____
Write the oxidation half reaction: _____________________________
Write the reduction half reaction: _____________________________
Write the balanced half reaction: ______________________________
Voltaic Cell review
Notation of voltaic cells:
Example:
Sodium (Na) is oxidized and nickel (Ni) is reduced
Oxidation half reaction: ______________________________
Reduction half reaction: ______________________________
Balanced half reaction:_______________________________
Cell notation:
Voltaic Cell basics

What is happening at the anode?

What is happening at the cathode?

What is the purpose of a salt bridge?

What is the purposed of the wire?
Draw what his happening in the cell below. Label the anode, the cathode, draw the direction in which
the electrons are traveling and be specific about what is happening at each of the electrodes (anode and
cathode). Magnesium is oxidized, copper (which in this solution is a 2+ ion) is reduced.
Oxidation half reaction:
Balanced reaction:
Reduction half reaction:
Cell notation:
For the following cell notation: Fe|Fe2+ || Ag+ | Ag
Write the half reaction occurring at the cathode: ____________________________
Write the half reaction occurring at the anode: _____________________________
Write the balanced reaction: ________________________________
Write the cell notation for a voltaic cell with the following half reactions:
Al  Al3+ + 3e-
Sn2+ + 2e-  Sn